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Electrochemical equivalent of $Cu$ in the reaction ${Cu}^{+ 2} + 2 e^{-} \to Cu$ is:

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Important Questions on Electrochemistry

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

How long (approximate) should water be electrolysed by passing through

100

amperes

current so that the oxygen released can completely burn

27.66 g

of diborane? (Atomic weight of

B = 10.8 u

)

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

Two Faraday of electricity is passed through a solution of

C u S O_{4}

. The mass of copper deposited at the cathode is: (Atomic mass of Cu = 63.5 amu)

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

A current of $10.0 A$ flows for $2.00 h$ through an electrolytic cell containing a molten salt of metal $X$ . This results in the decomposition of $0.250 mol$ of metal $X$ at the cathode. The oxidation state of $X$ in the molten salt is:

$(F = 96, 500 C)$

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

A solution of

N i {(N O_{3})}_{2}

is electrolyzed between platinum electrode

0.1

Faraday electricity. How many mole of

N i

will be deposited at the cathode?

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

When 9.65 ampere current was passed for 1.0 hour into nitrobenzene in acidic medium, the amount of p-aminophenol produced is:

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

108 g

of silver (molar mass

108 g {m o l}^{- 1}

) is deposited at cathode from

{A g N O}_{3} (a q)

solution by a certain quantity of electricity. The volume (in

L

) of oxygen gas produced at

273 K

and

1

bar pressure from water by the same quantity of electricity is

\frac{x}{10}

. Value of

' x'

to the nearest integer is _____.

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

The density of metal and equivalent weight of a metal are

10.5 g {cm}^{- 3}

and

100

, respectively. The time required for a current of

3 amp

to deposit a

0.005 mm

thick layer of the same metal on an area of

80 {cm}^{2}

is closest to

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

One litre solution of

{MgCl}_{2}

is electrolyzed completely by passing a current of

1 A

for

16 \min 5

sec. The original concentration of

{MgCl}_{2}

solution was (Atomic mass of

Mg = 24

)

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

For electroplating,

1.5 amp

current is passed for

250 s

through

250 m L of 0.15 M

solution of

M S O_{4} .

Only

85 %

of the current was utilised for electrolysis. The molarity of

M S O_{4}

solution after electrolysis is closest to [Assume that the volume of the solution remain constant]

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

Calculate the molarity of a solution containing

5 g

N a O H

dissolved in the product of a

H_{2} - O_{2}

fuel cell operated at

1 A

current for

595.1

hours.

(Assume

1 F = 96500 C / m o l

of electrons and molecular weight of

N a O H

40 g m o l^{- 1}

)

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

The weight of silver (at.wt.

= 108

) displaced by a quantity of electricity which displaces

5600 m L

O_{2}

STP

will be

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

During the electrolysis of molten sodium chloride, the time required to produce

0.10 mol

of chlorine gas using a current of

3 amperes

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

When

0.1 m o l {M n O}_{4}^{2 -}

is oxidized the quantity of electricity required to completely

M n O_{4}^{2 -}

M n O_{4}^{-}

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

Oxidation of succinate ion produces ethylene and carbon dioxide gases. On passing

0.2

Faraday electricity through an aqueous solution of potassium succinate, what is the total volume of gases (at both cathode and anode) at STP (

1 atm

and

273 K

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

An aqueous solution of

{CuSO}_{4}

is subjected to electrolysis using inert electrodes. The

pH

of the solution will

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

Potassium chlorate is prepared by the electrolysis of

KCl

in basic solution

6 {OH}^{-} + {Cl}^{-} \to {ClO}_{3}^{-} + 3 H_{2} O + 6 e^{-}

. If only

60 %

of the current is utilized in the reaction, the time (rounded to the nearest hour) required to produce

10 g

{KClO}_{3}

using a current of

2 A

\dots \dots . .

(Given :

F = 96, 500 C

mol

; molar mass of

{KClO}_{3} = 122 g {mol}^{- 1}

)

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

An acidic solution of dichromate is electrolysed for $8$ minutes using $2$ A current. As per the following equation

${Cr}_{2} O_{7}^{2 -} + 14 H^{+} + 6 e^{-} \to 2 {Cr}^{3 +} + 7 H_{2} O$
The amount of ${Cr}^{3 +}$ obtained was $0.104 g$ . The efficiency of the process $(in %)$ is (Take : $F = 96000 C$ , At. mass of chromium $= 52$ )

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

A solution of

N i {(N O_{3})}_{2}

is electrolyzed between platinum electrodes using a current of

5

amperes for

20

minutes. What mass of

N i

is deposited at the cathode?

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

The number of electrons delivered at the cathode, during electrolysis by a current of

1 ampere in 60 seconds

is (charge on electron

= 1.60 \times 10^{- 19} C

)

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrolytic Cells

A constant current (0.5 amp) is passed for 1 hour through (i) aqueous

A g N O_{3}

. (ii) aqueous

C u S O_{4}

and (iii) molten

A l F_{3}

, separately. The ratio of the mass of the metals deposited on the cathode is

[M_{Ag}, M_{Cu}, M_{Al}

are molar masses of the respective metals

]

Electrochemical equivalent of Cu in the reaction Cu+2 + 2e− → Cu is:

Important Questions on Electrochemistry

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Electrochemical equivalent of $Cu$ in the reaction ${Cu}^{+ 2} + 2 e^{-} \to Cu$ is: